Magnesium»the essentials [WebElements Periodic Table] Magnesium tarnishes slightly in air, and finely divided magnesium readily ignites upon heating in air and burns with a dazzling white flame. Normally magnesium is coated with a layer of oxide, MgO, that protects magnesium from air and water. Magnesium: historical information Magnesium was discovered by Sir Humphrey Davy in 1755 at England. Origin of name : from the Greek word "Magnesia", a district of Thessaly. In 1618 a farmer at Epsom in England attempted to give his cows water from a well. This they refused to drink because of the water's bitter taste. However the farmer noticed that the water seemed to heal scratches and rashes. The fame of Epsom salts spread. Eventually they were recognised to be magnesium sulphate, MgSO4. Black recognized magnesium as an element in 1755. It was isolated by Davy in 1808 who electrolysed a mixture of magnesia (magnesium oxide, MgO) and mercuric oxide (HgO). Davy's first suggestion for a name was magnium but the name magnesium is now used.

Sometime prior to the autumn of 1803, the Englishman John Dalton was able to explain the results of some of his studies by assuming that matter is composed of atoms and that all samples of any given compound consist of the same combination of these atoms. Dalton also noted that in series of compounds, the ratios of the masses of the second element that combine with a given weight of the first element can be reduced to small whole numbers (the law of multiple proportions). This was further evidence for atoms. Dalton's theory of atoms was published by Thomas Thomson in the 3rd edition of his System of Chemistry in 1807 and in a paper about strontium oxalates published in the Philosophical Transactions. Dalton published these ideas himself in the following year in the New System of Chemical Philosophy. The symbol used by Dalton for magnesium is shown below. [See History of Chemistry, Sir Edward Thorpe, volume 1, Watts & Co, London, 1914.] Magnesium around us Read more » Magnesium is an important element for plants and animals. Chlorophylls (responsible for the green colour of plants) are compounds knonw as porphyrins and are based upon magnesium.

Magnesium is required for the proper working of some enzymes. The adult daily requirement of magnesium is about 0.3 g day-1. Magnesium is the eighth most abundant element in the earth's crust but is never found as the free metal. There are many minerals containing magnesium including magnesite and dolomite. Sea water also contains plenty of magnesium. Abundances for magnesium in a number of different environments. More abundance data » Location Second ionisation energy : 1450.7 kJ mol‑1 Isolation Isolation : magnesium can be made commercially by several processes and would not normally be made in the laboratory because of its ready availability. There are massive amounts of magnesium in seawater. This can be recovered as magnesium chloride, MgCl2 through reaction with calcium oxide, CaO. CaO + H2O → Ca2+ + 2OH- Mg2+ + 2OH- → Mg(OH)2 Mg(OH)2 + 2HCl → MgCl2 + 2H2O Electrolysis of hot molten MgCl2 affords magnesium as a liquid whih is poured off and chlorine gas.

cathode: Mg2+(l) + 2e- → Mg anode: Cl-(l) → 1/2Cl2 (g) + e- The other methos used to produce magnesium is non electrolytic and involves dolomite, [MgCa(CO3)2], an important magnesium mineral. This is "calcined" by heating to form calcined dolomite, MgO.CaO, and this reacted with ferrosilicon alloy. 2[MgO.CaO] + FeSi → 2Mg + Ca2SiO4 + Fe The magnesium may be distilled out from this mixture of products. Magnesium isotopes Magnesium (Mg) - Chemical properties, Health and Environmental effects Magnesium Chemical element, metallic, symbol Mg, situated in group IIa in the periodic table, atomic number: 12, atomic weight: 24,312. Magnesium is silvery white and very light. Its relative density is 1,74 and it’s density 1740 kg/m3 (0.063 lb/in3 or 108.6 lb/ft3).

Magnesium is known for a long time as the lighter structural metal in the industry, due to it’s low weight and to it’s capability of forming mechanically resistant alloys. Magnesium is very chemically active, it takes the place of hydrogen in boiling water and a great number of metals can be produced by thermic reduction of its salts and oxidized forms with magnesium. It joins together with most non-metals and almost every acid. Magnesium reacts only slightly or not at all with most of the alkalis and many organic substances, like hydrocarbons, aldehides, alcohols, phenols, amines, esters and most of the oils. Used as a catalyst, magnesium promotes organic reactions of condensation, reduction, addition and dehalogenization. It was used for a long time for synthesizing special and complex organic components by the well-known Grignard reaction. The main ingredients of the alloys are: aluminum, manganese , zircon , zinc , rare-earth metals and thorium . Applications Magnesium compounds are used as refractory material in furnace linings for producing metals (iron and steel, nonferrous metals), glass, and cement.

With a density of only two thirds of the aluminum ’s, it has countless applications in cases where weight reducing is important, i.e. in aeroplane and missile construction. It also has many useful chemical and metallurgic properties, which make it appropriate for many other non-structural applications. Magnesium components are widely used in industry and agriculture. Other uses include: removal of sulphur form iron and steel, photoengraved plates in the printing industry; reducing agent for the production of pure uranium and other metals from their salts; flashlight photography, flares, and pyrotechnics. Magnesium in the environment Magnesium is the eighth most abundant element and constitutes about 2% af the Earth's crust by weight, and it is the third most plentiful element dissolved in seawater. It’s very abundant in nature, and it’s found in important quantities in many rocky minerals, like dolomite, magnetite, olivine and serpentine. It’s also found in seawater, underground brines and salty layers. It’s the third most abundant structural metal in the earth’s crust, only exceeded by aluminum and iron .

The United States has traditionally been the major world supplier of this metal, supplying 45% of world production even as recently as 1995. Dolomite and magnesite are mined to the extent of 10 million tonnes per year, in countries such as China, Turkey, North Korea, Slovakia, Austria, Russia and Greece. Health effects of magnesium Humans take in between 250 and 350 mg/day of magnesium and need at least 200 mg, but the body deals very effectively with this element, taking it form food when it can, and recycling what we already have when it cannot. There is no evidence that magnesium produces systemic poisoning although persistent over-indulgence in taking magnesium supplements and medicines can lead to muscule weakness, lethargy and confusion. Effects of exposure to magnesium powder: low toxicity & not considered to be hazardous to health. Inhalation: dust may irritate mucous membranes or upper respiratory tract. Eyes: mechanical injury or particle may embed in eye. Viewing of burning magnesium powder without fire glasses may result in "Welder's flash", due to intense white flame. Skin: embedding of particle in skin.

Ingestion: unlikely; however, ingestion of large amounts of magnesium powder could cause injury. Magnesium has not been tested, but it’s not suspected of being carcinogenic, mutagenic or teratogenic. Exposure to magnesium oxide fume subsequent to burning, welding or molten metal work can result in metal fume fever with the following temporary symptoms: fever, chills, nausea, vomiting & muscle pain. These usually occur 4-12 hours after exposure & last up to 48 hours. Magnesium oxide fume is a by-product of burning magnesium. Physical dangers: Dust explosion possible if in powder or granular form, mixed with air. If dry, it can be charged electrostatically by swirling, pneumatic transport, pouring, etc. Chemical dangers: The substance may spontaneously ignite on contact with air or moisture producing irritating or toxic fumes. Reacts violently with strong oxidants. Reacts violently with many substances causing fire and explosion hazard. Reacts with acids and water forming flammable hydrogen gas (see ICSC0001), causing fire and explosion hazard. First Aid: Inhalation: remove to fresh air. Eyes: flush eyes with water thoroughly. Consult a physician.

Skin: wash with soap & water thoroughly to remove particles. Ingestion: if large amounts of magnesium powder are ingested, induce vomiting & consult a physician. Note to physician: no specific treatment or antidote. Supportive care recommended. Treatment should be based on reactions of the patient. Environmental effects of magnesium There is very little information available on the environmental effects of magnesium oxide fume. If other mammals inhale magnesium oxide fume, they may suffer similar effects as do humans. On an environmental spectrum of 0 - 3 Magnesium oxide fume registers 0.8. A score of 3 represents a very high hazard to the environment and 0 a negligible hazard. Factors that are taken into account to obtain this ranking include the extent of the material's toxic or poisonous nature and/or its lack of toxicity, and the measure of its ability to remain active in the environment and whether it accumulates in living organisms. It does not take into exposure to the substance. Magnesium powder is not suspected of being highly harmful to the environment. As magnesium oxide an aquatic toxicity rating of tlm 1000 ppm has been established. "Water Quality Characteristics of Hazardous Materials", Hann & Jensen, Enviro. End.

Div., Texas A&M, vol. 3 (1974). Magnesium Facts - Periodic Table of the Elements Magnesium Facts Magnesium Facts Magnesium Chemical & Physical Properties Photograph of the element magnesium, with a penny to indicate size of the sample. U.S. Geological Survey Electron Configuration : [Ne] 3s2 Word Origin: Magnesia, a district in Thessaly, Greece Properties: Magnesium has a melting point of 648.8°C, boiling point of 1090°C, specific gravity of 1.738 (20°C), and valence of 2. Magnesium metal is light (one-third lighter than aluminum), silvery-white, and relatively tough. The metal tarnishes slightly in air. Finely divided magnesium ignites upon heating in air, burning with a bright white flame. Uses: Magnesium is used in pyrotechnic and incendiary devices. It is alloyed with other metals to make them lighter and more easily welded, with applications in the aerospace industry. Magnesium is added to many propellents . It is used as a reducing agent in the preparation of uranium and other metals that are purified from their salts.

Magnesite is used in refactories. continue reading below our video Test Your General Science Knowledge Magnesium hydroxide (milk of magnesia), sulfate (Epsom salts), chloride, and citrate are used in medicine. Organic magnesium compounds have many uses. Magnesium is essential for plant and animal nutrition. Chlorophyll is a magnesium-centered porphyrin. Sources: Magnesium is the 8th most abundant element in the earth's crust. While it is not found free it nature, it is available in minerals including magnesite and dolomite. The metal may be obtained by electrolysis of fused magnesium chloride derived from brines and seawater. Chemical Elements.com - Magnesium (Mg) Contains an "Introduction to Tungsten", among other things If you know of any other links for Magnesium, please let me know Bentor, Yinon. Chemical Element.com - Magnesium. < For more information about citing online sources, please visit the MLA's Website . This page was created by Yinon Bentor. Use of this web site is restricted by this site's license agreement . Copyright © 1996-2012 Yinon Bentor. All Rights Reserved.

Is magnesium a metal, nonmetal or metalloid? | Reference.com Is magnesium a metal, nonmetal or metalloid? A: Quick Answer Magnesium is classified as an alkaline earth metal. Metals are defined as elements that can be hammered into sheets (malleable), made into a wire (ductile) and are good conductors of electricity and heat. Full Answer The chemical symbol of magnesium is Mg, and it has an atomic number of 12. As a solid, the element has a shiny, gray appearance, which is one of the characteristics of elements in the metal group on the periodic table. It is highly flammable, especially when shaved or in the form of a powder. Once lit, it is difficult to extinguish as it can burn in nitrogen, carbon dioxide and water. While magnesium only occurs naturally in combination with other elements, it remains the ninth most abundant element in the universe, the eighth most abundant in the Earth's crust and the fourth most common element in the Earth itself. Magnesium makes up 13 percent of the Earth's mass. In humans, Magnesium ions are essential to various functions in all cells.

In fact, by mass, the element is the 11th most abundant element in the human body. Magnesium ions interact with compounds like DNA, RNA and ATP. The element is also used for medicinal purposes. For example, laxatives and antacids use magnesium, and it is also used to stabilize abnormal blood vessel spasms or nerve excitation. Magnesium - Element information, properties and uses | Periodic Table Chemistry in its element: magnesium (Promo) You're listening to Chemistry in its element brought to you by Chemistry World, the magazine of the Royal Society of Chemistry (End promo) Chris Smith Hello, this week we meet the substance whose chemical claim to fame is that its quite literally hit a bum note in the past as a cure for constipation. But its explosive role isn't just confined to the colon because it's also the basis of incendriary bombs and even the existence of life on earth. And to tell the story of Magnesium, here's John Emsley.

John Emsley It was once the destroyer of cities - now it's a saver of energy The summer of 1618 saw England gripped by drought, but as Henry Wicker walked across Epsom Common he was came across a pool of water from which thirsty cattle refused to drink. He found that the water tasted bitter and on evaporation it yielded a salt which had a remarkable effect: it acted as a laxative. This became the famous Epsom's salt (magnesium sulfate, MgSO4) and became a treatment for constipation for the next 350 years. The first person to propose that magnesium was an element was Joseph Black of Edinburgh in 1755, and an impure form of metallic magnesium was produced in 1792 by Anton Rupprecht who heated magnesia (magnesium oxide, MgO) with charcoal. He named the element austrium after his native Austria. A small sample of the pure metal was isolated by Humphry Davy in 1808, by the electrolysis of moist MgO, and he proposed the name magnium based on the mineral magnesite (MgCO3) which came from Magnesia in Greece.

Neither name survived and eventually it was called magnesium. Magnesium is essential to almost all life on Earth - it is at the heart of the chlorophyll molecule, which plants use to convert carbon dioxide into glucose, and then to cellulose, starch, and many other molecules which pass along the food chain. Humans take in around 300 mg of magnesium per day and we need at least 200 mg, but the body has a store of around 25 g of this element in its skeleton so there is rarely a deficiency. Almonds, brazil nuts, cashew nuts, soybeans, parsnips, bran, and even chocolate are all rich in magnesium. Some brands of beer contain a lot, such as Webster's Yorkshire Bitter - it may owe some of its flavour to the high levels of magnesium sulfate in the water used to brew it. Magnesium is the seventh most abundant element in the Earth's crust, and third most abundant if the Earth's mantle is also taken into consideration because this consists largely of olivine and pyroxene, which are magnesium silicates.

It is also abundant in sea water (1200 p.p.m.) so much so that this was the source of magnesium for bombs in World War II. The metal itself was produced by the electrolysis of the molten chloride. Once magnesium starts to burn it is almost impossible to extinguish, because it reacts exothermically with oxygen, nitrogen and water. It burns with a bright light and was used for photographic flash bulbs It made an ideal incendiary agent and in some air raids during World War II as many as half a million 2 kg magnesium bombs would be scattered over a city in the space of an hour. The result was massive conflagrations and firestorms. Bulk magnesium metal is not easily ignited so this had to be done by a thermite reaction at the heart of the bomb. The thermite reaction, between aluminium powder and iron oxide, releases more than enough heat to cause the magnesium casing of the bomb to burn fiercely. Many minerals are known which contain magnesium; but the main ones are dolomite (calcium magnesium carbonate, CaMg(CO3)2) and magnesite which are mined to the extent of 10 million tonnes per year.

Magnesite is heated to convert it to magnesia (MgO), and this has several applications: fertilizers; cattle feed supplement; a bulking agent in plastics; and for heat-resistant bricks for fireplaces and furnaces. The metal itself is being produced in increasing amounts. It was originally introduced for racing bicycles which were the first vehicles to use pure magnesium frames, giving a better combination of strength and lightness than other metals. (A steel frame is nearly five times heavier than a magnesium one.) For use as a metal, magnesium is alloyed with a few percent of aluminium, plus traces of zinc and manganese, to improve strength, corrosion resistance and welding qualities, and this alloy is used to save energy by making things lighter. It is found in car and aircraft seats, lightweight luggage, lawn mowers, power tools, disc drives and cameras. At the end of its useful life the magnesium in all these products can be recycled at very little cost. Because it is an electropositive metal, magnesium can be act as a 'sacrificial' electrode to protect iron and steel structures because it corrodes away preferentially when they are exposed to water which otherwise would cause rusting Chris Smith So better bikes, better bombs and better bums.

Thank you very much to science writer John Emsley for telling the tale of Magnesium. Next week the illuminating story of the element that spawned a light bulb but really needs to work on its image. Quentin Cooper If any element needs a change of PR this is the one. It's brittle, prone to ponginess and arguably the dunce of the periodic table. Even the man who discovered osmium treated it rather sniffily. It reeked - or at least some of its compounds did. Tennant described the "pungent and penetrating smell" as one of the new element's "most distinguishing characters". So he called it osmium - osme being the Greek for odour. Chris Smith That's Quentin Cooper who will be undressing osmium for us in next week's Chemistry in its element, I hope you can join us. I'm Chris Smith, thank you for listening, see you next time. (Promo) Chemistry in its element is brought to you by the Royal Society of Chemistry and produced by thenakedscientists.com . There's more information and other episodes of Chemistry in its element on our website at chemistryworld.org/elements .

(End promo) Metal Metal - Selenium Lithium Lithium is a soft, silver-white metal that belongs to the alkali metal group of chemical elements. It is represented by the symbol Li, and it has the atomic number three. » request a quote Potassium Potassium is the chemical element with the symbol K (Latin: kalium, from Arabic: al-qalyah plant ashes, cf. Alkali from the same root), atomic number 19, and atomic mass 39.0983. Potassium was first isolated from potash. » request a quote Sodium Sodium is a metallic element with a symbol Na (from Latin natrium or Arabic natrun) and atomic number 11. It is a soft, silvery-white, highly reactive metal and is a member of the alkali metals within "group 1" (formerly known as group IA). It has only one stable isotope, 23Na. » request a quote Zinc Zinc also known as spelter, is a metallic chemical element; it has the symbol Zn and atomic number 30. It is the first element in group 12 of the periodic table.

Zinc is, in some respects, chemically similar to magnesium, because its ion is of similar size and its only common oxidation state is +2. » request a quote Vanadium Vanadium is the chemical element with the symbol V and atomic number 23. It is a soft, silvery grey, ductile transition metal. The formation of an oxide layer stabilizes the metal against oxidation. » request a quote Calcium Calcium is the chemical element with the symbol Ca and atomic number 20. It has an atomic mass of 40.078 amu. Calcium is a soft gray alkaline earth metal, and is the fifth most abundant element by mass in the Earth's crust. » request a quote Barium Barium is a chemical element. It has the symbol Ba, atomic number 56, and is the fifth element in Group 2. Barium is a soft silvery metallic alkaline earth metal. It is never found in nature in its pure form due to its reactivity with air. Its oxide is historically known as baryta but it reacts with water and carbon dioxide and is not found as a mineral.

» request a quote Magnesium Magnesium is a chemical element with the symbol mg, atomic number 12 and common oxidation number +2. It is an alkaline earth metal and the eighth most abundant element in the earth's crust by mass, although ninth in the universe as a whole. Naming Chemical Compounds & Writing Chemical Formulas Binary Compounds All true binary compounds contain only two elements. The name of every binary compound ends with ï¿½ide.ï¿½ Binary compounds come in three types. They are: Type I............. the metal forms only one type of cation Type II............ the metal forms two or more types of cations Type III.......... contains only nonmetals We will look at each type, one at a time. Type I Binary Compounds For Type I binary compounds the metal present can be found in either Group 1 or Group 2 on the periodic table. The naming system for this type of compound is quite simple and is found below. Rules for naming Type I binary compounds 1. The cation is always named first and the anion second. 2. A simple cation (obtained from a single atom) takes its name from the name of the element. 3.

A simple anion (obtained from a single atom) is named by taking the first part of the element name (the root) and adding the letters ï¿½IDE.ï¿½ 4. Write the name for the compound by combining the names of the ions. Name the compound RbI. ï¿½ Rb is the chemical symbol for rubidium. ï¿½ I is the chemical symbol for iodine, whose root is ï¿½iod.ï¿½ Add the ï¿½ideï¿½ ending to get iodide. ï¿½ Put the pieces together to get the name rubidium iodide. Name the compound CaO. ï¿½ Ca is the chemical symbol for calcium. ï¿½ O is the symbol for oxygen, whose root is ï¿½ox.ï¿½ Add the ï¿½ideï¿½ ending to get oxide. ï¿½ Put the pieces together to get the name calcium oxide. Name the compound Li3N. ï¿½ Li is the chemical symbol for lithium.

ï¿½ N is the chemical symbol for nitrogen, whose root is ï¿½nitr.ï¿½ Add the ï¿½ideï¿½ ending to get nitride. ï¿½ Put the pieces together to get the name lithium nitride. Write the formula for potassium sulfide. ï¿½ The chemical symbol of potassium is K. K is in the 1st column of the periodic table, therefore, its oxidation state is +1. ï¿½ Sulfide is derived from sulfur, whose symbol is S. Its oxidation state is -2. +1 -2 ï¿½ So far we haveï¿½ K S. ï¿½ The total positive charge must balance the total negative charge. Therefore, we need 2 K atoms to give a total positive charge of +2. This balances the -2 charge on the sulfur. ï¿½ Putting it all together we have K2S. Write the formula for magnesium chloride. ï¿½ The chemical symbol of magnesium is Mg. Mg is in the 2nd column of the periodic table, therefore, its oxidation state is +2. ï¿½ Chloride is derived from chlorine, whose symbol is Cl. Its oxidation state is -1.

+2 -1 ï¿½ So far we haveï¿½ Mg Cl ï¿½ The total positive charge must balance the total negative charge. Therefore, we need 2 chlorine atoms to give a total negative charge of -2. This balances the charge on the magnesium. ï¿½ Putting it all together we have MgCl2. NaCl ï¿½ sodium chloride KI ï¿½ potassium iodide RbBr ï¿½ rubidium bromide MgS ï¿½ magnesium sulfide Mg3N2 ï¿½ magnesium nitride Sodium fluoride ï¿½ NaF Strontium oxide ï¿½ SrO Beryllium chloride ï¿½ BeCl2 Cesium sulfide ï¿½ Ce2S Potassium phophide ï¿½ K3P Type II Binary Compounds For Type II binary compounds the metal present is NOT found in either Group 1 or Group 2 on the periodic table. The naming system for this type of compound is found below. Rules for naming Type II binary compounds 1. The cation is always named first and the anion second. 2.

A simple cation (obtained from a single atom) takes its name from the name of the element. Include a Roman numeral to indicate the oxidation number (charge) on the metal cation. 3. A simple anion (obtained from a single atom) is named by taking the first part of the element name (the root) and adding the letters ï¿½IDE.ï¿½ 4. Write the name for the compound by combining the names of the ions. Name the compound FeCl2. ï¿½ Fe is the chemical symbol for iron. o Fe is not in the 1st or 2nd column; therefore a Roman numeral is needed in the name. Weï¿½ll come back to that shortly. ï¿½ Cl is the chemical symbol for chlorine, whose root is ï¿½chlor.ï¿½ Add the ï¿½ideï¿½ ending to get chloride. ï¿½ At this point we have iron (??) chloride. ï¿½ To find the Roman numeralï¿½ o Find the charge of the anion. ï¿½ Cl has a -1 charge. o Multiply times the number of those atoms to get the total negative charge.

ï¿½ There are 2 Cl atoms. ï¿½ 2 times -1 = -2. <--- total negative charge. o Balance total negative charge with total positive charge. ï¿½ The total negative charge of -2 must be balanced with a total positive charge of +2. o Divide the total positive charge by the number of atoms to get Roman numeral. ï¿½ There is only 1 Fe ï¿½ +2 divided by 1 = +2. The Roman numeral is II. ï¿½ Put the pieces together to get the name iron (II) chloride. Name the compound PbS2. ï¿½ Pb is the chemical symbol for lead. o Pb is not in the 1st or 2nd column; therefore a Roman numeral is needed. ï¿½ S is sulfur, whose root is ï¿½sulf.ï¿½ Add the ï¿½ideï¿½ ending to get sulfide. ï¿½ At this point we have lead (??) sulfide. ï¿½ To find the Roman numeralï¿½ ï¿½ S has a charge of -2. ï¿½ There are 2 sulfur atoms soï¿½.

2 x -2 = -4. <---- total negative charge ï¿½ The total positive charge must be +4. ï¿½ There is 1 lead atom soï¿½ +4 ï¿½ 1 = +4. The Roman numeral is IV. ï¿½ Put the pieces together to get the name lead (IV) sulfide. Write the formula for nickel (III) oxide. ï¿½ The chemical symbol of nickel is Ni. The oxidation state is +3, as given by the Roman numeral. ï¿½ Oxide is derived from oxygen, whose symbol is O. Its oxidation state is -2. +3 -2 ï¿½ So far we have Ni O. ï¿½ In order to balance the charges we find the least common multiple (LCM) of 3 and 2. The LCM is 6. We need two Ni atoms (+6 ï¿½ +3 = 2) and three O atoms (-6 ï¿½ -2 = 3) to balance the charges. ï¿½ Putting it all together we have Ni2O3. Write the formula for lead (IV) nitride. ï¿½ The chemical symbol of lead is Pb.

The oxidation state is +4. ï¿½ Nitride is derived from nitrogen, whose symbol is N. Its oxidation state is -3. +4 -3 ï¿½ So far we have Pb N. ï¿½ The LCM of 4 and 3 is 12. We need three Pb atoms (+12 ï¿½ +4 = 3) and 4 N atoms (-12 ï¿½ -3 = 4) to balance the charges. ï¿½ Putting it all together we have Pb3N4. Write the name for iron (II) oxide. ï¿½ The chemical symbol of iron is Fe. The oxidation state is +2. ï¿½ Oxide is derived from oxygen, whose symbol is O. Its oxidation state is -2. +2 -2 ï¿½ So far we have Fe O ï¿½ Since the charges already balance there is no additional work to be done. ï¿½ Putting it all together we have FeO.

Fe2O3 ï¿½ Iron (III) oxide CuCl ï¿½ Copper (I) chloride CuCl2 ï¿½ Copper (II) chloride PbS ï¿½ lead (II) sulfide PbS2 ï¿½ lead (IV) sulfide Chromium (VI) oxide ï¿½ CrO3 Cobalt (III) sulfide ï¿½ Co2S3 Nickel (II) bromide ï¿½ NiBr2 Mercury (II) phosphide ï¿½ Hg3P2 Cadmium (II) iodide ï¿½ CdI2 Type III Binary Compounds Type III binary compounds contain no metal atoms. There are two different naming systems for Type III binary compounds: the ï¿½old systemï¿½ and the ï¿½new system.ï¿½ The old system uses prefixes to indicate the number of each atom present and the new system is identical to that used for naming Type II compounds. It is important to note that only one system can be used at a time. NEVER mix prefixes and Roman numerals. Rules for naming Type III binary compounds: the OLD SYSTEM 1.

The first element in the formula is named first, and the full element name is used. 2. The second element is named as though it were an anion: root + ide 3. Prefixes are used to denote the numbers of atoms present. (See table below) 4. The prefix mono- is never used for naming the first element. Name the compound NO2. ï¿½ N is the chemical symbol of nitrogen. Since there is only one nitrogen atom AND it is the first element the prefix mono is not used. ï¿½ O is the chemical symbol of oxygen, whose root is ox. Add the ide ending to get oxide. There are two oxygen atoms so we also add the prefix di to get dioxide. ï¿½ Put the pieces together to get the name nitrogen dioxide. Name the compound N2O. ï¿½ N is the chemical symbol of nitrogen. Since there are two nitrogen atoms we need to add the prefix di to get dinitrogen. ï¿½ O is the chemical symbol of oxygen, whose root is ox. Add the ide ending to get oxide. There is only one oxygen atom we add the prefix mono (mono IS used for the second element) to get monoxide.

ï¿½ Put the pieces together to get the name dinitrogen monoxide. Write the formula for carbon tetrachloride. ï¿½ The chemical symbol of carbon is C. There is no prefix before carbon in the chemical name, therefore, there is only 1 C atom in the chemical formula. ï¿½ Tetrachloride has the prefix tetra which means there are 4 atoms present. Chloride is derived from chlorine, whose symbol is Cl. Thus, there are 4 Cl atoms in the chemical formula. ï¿½ Putting it all together we have CCl4. Write the formula for dinotrogen pentaoxide. ï¿½ The prefix di means 2. Thus there are 2 N atoms in the chemical formula. ï¿½ The prefix penta means 5. Thus, there are 5 O atoms in the chemical formula. ï¿½ Putting it all together we have N2O5. Now let us apply the ï¿½new systemï¿½ to these same compounds. For Type III binary compounds the ï¿½new systemï¿½ is identical to that used to name Type II binary compounds.

The advantage to using the new system is that you have one less system to learn. Rules for naming Type III binary compounds: the NEW SYSTEM 1. The cation is always named first and the anion second. 2. A simple cation (obtained from a single atom) takes its name from the name of the element. Include a Roman numeral to indicate the oxidation number (charge) on the metal cation. 3. A simple anion (obtained from a single atom) is named by taking the first part of the element name (the root) and adding the letters ï¿½IDE.ï¿½ 4. Write the name for the compound by combining the names of the ions. Name the compound NO2. ï¿½ N is the chemical symbol for nitrogen. o Nitrogen is not in the 1st or 2nd column; therefore a Roman numeral is needed in the name. ï¿½ O is the symbol for oxygen, whose root is ï¿½ox.ï¿½ Add the ï¿½ideï¿½ ending to get oxide. ï¿½ At this point we have nitrogen (??) oxide.

ï¿½ To find the Roman numeralï¿½ ï¿½ O has a charge of -2. ï¿½ 2 oxygen atoms times -2 = -4. <---- total negative charge. ï¿½ The total negative charge of -4 must be balanced with a total positive charge of +4. ï¿½ +4 divided by 1 (one N atom) = +4. The Roman numeral is IV. ï¿½ Put the pieces together to get the name nitrogen (IV) oxide. Name the compound N2O. ï¿½ N is the chemical symbol for nitrogen. o Nitrogen is not in the 1st or 2nd column; therefore a Roman numeral is needed in the name. ï¿½ O is the symbol for oxygen, whose root is ï¿½ox.ï¿½ Add the ï¿½ideï¿½ ending to get oxide. ï¿½ At this point we have nitrogen (??) oxide. ï¿½ To find the Roman numeralï¿½. ï¿½ O has a charge of -2. ï¿½ 2 oxygen atoms times -2 = -4. <---- total negative charge. ï¿½ The total positive charge must be +2.

ï¿½ +2 divided by 2 (2 N atoms) = +1. The Roman numeral is I. ï¿½ Put the pieces together to get the name nitrogen (I) oxide. Write the formula for carbon(IV) chloride. ï¿½ The symbol for carbon is C. The oxidation state is +4, as given by the Roman numeral. ï¿½ Chloride is derived from chlorine. The charge on chlorine is -1. +4 -1 ï¿½ So far we have C Cl ï¿½ The LCM of 4 and 1 is 4. We need 1 C atom (+4 ï¿½ +4 = 1) and 4 Cl atoms (-4 ï¿½ -1 = 4) to balance the charges. ï¿½ Putting it all together we have CCl4. Write the formula for nitrogen (V) oxide. ï¿½ The symbol for nitrogen is N. The Roman numeral indicates a charge of +5. ï¿½ Oxide is derived from oxygen. The charge on oxygen is -2.

+5 -2 ï¿½ So far we have N O ï¿½ The LCM of 5 and 2 is 10. Therefore, we need 2 N atoms and 5 O atoms to balance the charges. ï¿½ Putting it all together we have N2O5. (A.K.A. Compounds that contain polyatomic ions) An ion is an atom with an electric charge (positive or negative). A polyatomic ion is a group of atoms with an electric charge. (Even though it is a group of atoms it acts like it were a single atom.) The names of nearly all polyatomic ions end with the letters ï¿½ate or ï¿½ite. Beware three exceptions: cyanide, hydroxide, and peroxide. These ions end with ï¿½ideï¿½ which can trick into thinking you have a binary compound when you actually have a ternary compound. Follow the naming systems for Type I and Type II binary compounds butï¿½ DONï¿½T CHANGE THE NAME OF THE POLYATOMIC ION.

Na2SO4 ï¿½ sodium sulfate KH2PO4 ï¿½ potassium dihydrogen phosphate Fe(NO3)3 ï¿½ iron (III) nitrate Mn(OH)2 ï¿½ manganese (II) hydroxide Na2SO3 ï¿½ sodium sulfite Calcium hydroxide ï¿½ Ca(OH)2 Sodium phosphate ï¿½ Na3PO4 Ammonium dichromate ï¿½ (NH4)2Cr2O7 Cobalt (II) perchlorate ï¿½ Co(ClO4)2 Copper (II) nitrite ï¿½ Cu(NO2)2 Naming Polyatomic Ions that Contain Oxygen There are many atoms that form several different polyatomic ions with oxygen. The naming system for these ions is based on two things: the most common ion in each series and the number of oxygen atoms compared to the most common ion. The ones that concern us most are ions of phosphorus, sulfur, nitrogen, chlorine, and carbon. Memorize these ions!

SO22- = hyposulfite Note: Some of the ions do not exist in the real world, they are written here to show how to use the naming system. Naming Acids For this class, ALL acids begin with H (hydrogen). The names of ALL acids end with the word ï¿½acid.ï¿½ There are two types of acids: those that contain oxygen and those that do not. Naming acids that DO NOT contain oxygen 1. Take the name of the anion, add the prefix ï¿½hydroï¿½ and change the ending to ï¿½ic.ï¿½ 2. Add the word ï¿½acid.ï¿½ Name the compounds HF. ï¿½ We know this is an acid because the chemical formula starts with ï¿½H.ï¿½ ï¿½ Take the name of the anion (fluoride) add the prefix ï¿½hydroï¿½ and change the ending to ï¿½icï¿½: hydrofluoric ï¿½ Finally, add the word ï¿½acid.ï¿½ ï¿½ hydrofluoric acid Name the compound HCN.

ï¿½ We know this is an acid because the chemical formula starts with ï¿½H.ï¿½ ï¿½ There is no oxygen present so we start with the prefix ï¿½hydro.ï¿½ ï¿½ Next, take the name of the anion (cyanide) and change the ending to ï¿½icï¿½: hydrocyanic ï¿½ Finally, add the word ï¿½acid.ï¿½ ï¿½ hydrocyanic acid Write the formula for hydrobromic acid. ï¿½ We know the formula starts with ï¿½Hï¿½ because it is an acid. The charge on hydrogen is +1. ï¿½ We also know that the acid does not contain oxygen because of the ï¿½hydroï¿½ prefix. ï¿½ Removing the ï¿½hydroï¿½ and ï¿½icï¿½ leaves us with ï¿½bromï¿½, the root of bromine or Br. The charge on bromine is -1. +1 -1 ï¿½ So far we have H Br ï¿½ Balance the charges to get the formula HBr.

Write the formula for hydrosulfuric acid. ï¿½ We know the formula starts with ï¿½Hï¿½ because it is an acid. The charge on hydrogen is +1. ï¿½ We also know that the acid does not contain oxygen because of the ï¿½hydroï¿½ prefix. ï¿½ Removing the ï¿½hydroï¿½ and ï¿½icï¿½ leaves us with sulfur. The charge on sulfur is -2. +1 -2 ï¿½ So far we have H S ï¿½ Balance the charges to get the formula H2S. Naming Acids the DO contain oxygen 1. Find the name of the polyatomic ion. 2. Change ï¿½ateï¿½ to ï¿½icï¿½ or ï¿½iteï¿½ to ï¿½ous.ï¿½ 3. Add the word acid. ï¿½ You know itï¿½s an acid because it starts with H. ï¿½ ClO4- is the perchlorate ion.

ï¿½ Change the ï¿½ateï¿½ to ï¿½icï¿½ and get perchloric. ï¿½ Add the word acid and get perchloric acid. ï¿½ You know itï¿½s an acid because it starts with H. ï¿½ SO32- is the sulfite ion. ï¿½ Change the ï¿½iteï¿½ to ï¿½ousï¿½ and get sulfous. ï¿½ Add the word acid and get sulfous acid. o The name is actually sulfurous acid, but I will count sulfous acid correct because it follows the naming system. Write the formula for phosphorous acid. ï¿½ The word acid tells us the first element is H. The charge on H is +1. ï¿½ We also know it is a ternary acid because the prefix ï¿½hydroï¿½ (meaning binary acid) is missing. ï¿½ Change ï¿½ousï¿½ to ï¿½iteï¿½ to get phophite. The formula for phophite is PO3-3. ï¿½ Putting it together and balancing the charges we get H3PO3.

Write the formula for each of the following compounds. 51. tin (II) nitrate 76. calcium bicarbonate 52. zinc (II) phosphate 77. calcium hydroxide 53. hypophosphorous acid 78. zinc (II) bisulfate 54. iron (III) chloride 79. silver (I) oxide 55. lithium sulfide 80. chlorous acid 56. silver (I) oxalate 81. lead (IV) oxide 57. perchloric acid 82. calcium acetate 58. potassium permanganate 83. sodium phosphate 59. strontium hypochlorite 84. copper (I) oxide 60. copper (I) sulfite 85. phosphorous acid 61. carbon (IV) sulfide 86. hydroiodic acid 62. calcium oxide 87. sodium fluoride 63. barium carbonate 88. phosphorus (V) oxide 64.

antimony (III) dichromate 89. sulfur (II) bromide 65. silicon (IV) oxide 90. aluminum (III) sulfate 66. iron (II) carbonate 91. nitrogen (III) oxide 67. sodium cyanide 92. aluminum (III) iodide 68. carbon (IV) chloride 93. iron (III) phosphate 69. cesium fluoride 94. zinc (II) perchlorate 70. sodium chromate 95. sodium dihydrogen phosphate 71. hydrosulfuric acid 96. sulfurous acid 72. aluminum (III) oxide 97. strontium carbonate 73. ammonium phosphate 98. copper (II) hydroxide 74. boron (III) fluoride 99. iron (II) oxalate 75. radium sulfate 100. phosphorous (V) sulfide

Question: Which metal has the chemical symbol Mg
Answer: Magnesium